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## Chem 113 Week 5

by: Caroline Hurlbut

13

0

2

# Chem 113 Week 5 Chem 113

Caroline Hurlbut
CSU
GPA 3.7

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These notes finish up with kinetics, covering concentration and rate constants as well as an intro to equilibrium
COURSE
General Chemistry II
PROF.
Ingrid Marie Laughman
TYPE
Class Notes
PAGES
2
WORDS
CONCEPTS
Chemistry
KARMA
25 ?

## Popular in Chemistry

This 2 page Class Notes was uploaded by Caroline Hurlbut on Friday February 19, 2016. The Class Notes belongs to Chem 113 at Colorado State University taught by Ingrid Marie Laughman in Spring 2016. Since its upload, it has received 13 views. For similar materials see General Chemistry II in Chemistry at Colorado State University.

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Date Created: 02/19/16
Concentration & Rate Constants • rate=k[A][B]^2 —reaction order is exponent of [A] + exponent of [B], or 1+2=3 —it can also be said that the reaction is ﬁrst order in A and second order in B —increasing concentration of reactants and/or the rate constant k can increase the rate of the reaction • Arrhenius equation: k=Ae^(-Ea/RT) —units of k depends on the order of the reaction • rearrangement of the Arrhenius equation —ln(k)=ln(A) - Ea/RT —in y-intercept form: ln(k)=-Ea/R(1/T) + ln(A) —for graph: 1/T (in K) on x axis, no units on y axis • zero order reactions —x—>products —rate=k[x]^0=k Zero Order First Order Second Order Example x—>products x—>products 2x—>products *rate does not depend *rate depends on [x]^1 on [x] Rate Law rate=-∆[x]/∆t=k0 rate=-∆[x]/∆t=k1[x] rate=(-1/2)∆[x]/ ∆t=k2[x]^2 Units of k M/S s^-1=1/s M^-1s^-1=1/Ms Integrated Rate Law [x]=-k0t + [x]0 ln(x)=-k1t + ln[x]0 -1/[x]=k2t + 1/[x]0 Plot time on x axis, [x] on y time on x axis, ln[x] ontime on x axis, 1/[x] on y axis, slope=-k0 axis, slope=-k1 axis, slope=k2 (positive (negative linear) (negative linear) linear) Half Life t(1/2)=[x]/2k 0.693/k 1/k[x]0 Intro to Equilibrium • reactants⁶products —forward rate=reverse rate • equilibrium is a constant state of movement and has nothing to do with the amount of reactants/products in a reaction —if there is a lot of product, the equilibrium leans to the right (direction of forward reaction) —if there is little product, the equilibrium leans to the left (direction of reverse reaction) • calculate equilibrium constant (K) = [B]^b/[A]^a = kf/kr —kf=forward rate constant —kr=reverse rate constant • calculate reaction quotient (Q) = [products]^coefﬁcient [reactants]^coefﬁcient —K and Q do not have units —Q tell us relative amounts of reactants and products —at equilibrium Q=K • special cases of K —Kc refers to concentration in terms of molarity —Kp refers to concentration in terms of partial pressure: Kp=PB^b/PA^a

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